100g of ice at -10C is placed into 100g of warm water in an insulated container.

Question

100g of ice at -10C is placed into 100g of warm water in an insulated container. The initial temperature of the water before the ice is added is 80C. A. What is the final temperature of the system? B. How much heat flowed from the warm water in the approach of equilibrium? C. Calculate the mass of the ice that remains when equilibrium is achieved. D. Calculate the change in entropy of the warm water as it cools in the approach to equilibrium. E. Calculate the change in entropy of the ice that warms to freezing and partially melts in the approach to equilibrium. F. Calculate the net change in entropy between the initial and final states of the system.

Explanation / Answer

heat required to convert ice from -10C to 0C=100*1*10=1000cal heat released when water at 80C converts to water at 0C=100*1*80=8000cal so,amount of ice melted=(8000-1000)/80=87.5g where 80cal/g is the latent heat of melting of ice so,mass of ice that remains=100-87.5=12.5g 1)final temperature=0 C 2)heat flowed from hot water=8000 cal 3)mass of ice that remains=12.5 g for hot water, dS=100*1*ln(273/353)=-25.699 cal/K for ice, dS=8000/273=29.30 cal/K for the system, dS=-25.699+29.30=3.605 cal/K

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